12 = 4 tops + 4 downs + 4 around
SF6, Sulfur hexafluorine: it is an S-centered octaedralform with 6 F at the 6 corners
6
8
8
This seems like a misprint. IF6 will have one electron too many to attain an octahedral structure with 90 degree bond angles. SF6 is octahedral, for example, and does have 90 degree angles, as does PF6(-1). Perhaps IF6(+1) is the molecule in question, which will have the proper number of electrons.
since it has a total of two atoms , its molecular shape is linear with bond angles of 180 degree.
It depends on what x and y are.
The bond angles are 120 degrees
Bond angle can be caused by internal angle between the orbitals having bonded pair of électrons, hybridization, presence of lone pair of electrons and electronegativity of the atom. and also Bond energy
This seems like a misprint. IF6 will have one electron too many to attain an octahedral structure with 90 degree bond angles. SF6 is octahedral, for example, and does have 90 degree angles, as does PF6(-1). Perhaps IF6(+1) is the molecule in question, which will have the proper number of electrons.
H2 dihydrogen only contains two atoms there is NO bond angle in a diatomic molecule.
When the central atom of a molecule has unshared electron, the bond angles will be less than when all the central atom's electrons are shared.
For a truly trigonal planar molecule the bond angles are 120 0 exactly.
the shape is linear and the bond angle is 180 degree
since it has a total of two atoms , its molecular shape is linear with bond angles of 180 degree.
Is tetrahedral with bond angles of 109.5 degree
trahedral
sp2 with 120 degree bond angles.
It depends on what x and y are.
the lone pair causes the molecule to become "bent" which makes the bond angles less than 109.5
It is formaldehyde in which carbon atom is sp2 hybridized so it is a triangular molecule with bond angles of 1200 .